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Chem 106 > Final Review > Flashcards

Final Review Flashcards

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1
Q

kinetic molecular theory

A

explains the behavior of gases based on the motion of their particles

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2
Q

what is a gases average kinetic energy proportional to?

A

absolute temp

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3
Q

what changes a gases volume?

A

temp and pressure

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4
Q

effusion

A

gas leaking through small holes from a high pressure area to a low pressure area

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5
Q

u

A

speed of molecules

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6
Q

smaller mass=

A

higher speed

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7
Q

absolute temperature

A

temp expressed on the Kelvin scale whose zero value is absolute zero

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8
Q

ideal gas

A

gas whose behavior is predicted by the linear relations defined by the combined gas law

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9
Q

STP Temp

A

273K

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10
Q

STP Pressure

A

1 atm

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11
Q

at STP, 1 mol of gas has a volume of…

A

22.4 L

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12
Q

molar volume=

A

v/n

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13
Q

density of gas

A

MP/RT

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14
Q

low molar mass means…

A

low density

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15
Q

what remains constant according to Boyle’s law?

A

temp and number of moles

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16
Q

what remains constant according to Charles law?

A

pressure and number of moles

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17
Q

what remains constant according to Amontom’s law?

A

volume and number of moles

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18
Q

what is constant according to the combined gas law?

A

number of moles

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19
Q

partial pressure

A

pressure of individual gases in a mixture

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20
Q

what finds partial pressure?

A

P1=xPtotal

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21
Q

what is the solubility of gases dependent on?

A

temp and pressure

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22
Q

as solubility increases…

A

pressure increases

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23
Q

as solubility decreases…

A

temp increases

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24
Q

what affects vapor pressure in liquids?

A

temp and intermolecular forces

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25
Q

vapor pressure

A

pressure exerted by a gas in equilibrium with liquid

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26
Q

what r do you use in the Clausius-clapeyron equation

A

8.3145

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27
Q

what does normal mean?

A

1 atm

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28
Q

how do you find total vapor pressure?

A

mole fraction * partial pressure

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29
Q

colligative properties

A

set of properties of a solution relative to the pure solvent

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30
Q

what do colligative properties depend on?

A

concentration of solute particles not identity

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31
Q

what is molality?

A

moles/kg of solvent

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32
Q

how does lattice energy affect solubility?

A

large lattice energy means limited solubility

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33
Q

volatile

A

having a significant vapor pressure at a given temp

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34
Q

what is the vapor pressure at a liquids normal boiling point?

A

1 atm

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35
Q

when is a liquid more volatile?

A

when it has a higher vapor pressure

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36
Q

why are theoretical and experimental values on van’t Hoffs factor different?

A

cations and anions cluster together and act as one molecule, this causes the fpd and bpe to be less than predicted

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37
Q

osmotic pressure

A

pressure applied across a semipermeable membrane to stop the flow

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38
Q

what does the kinetic molecular theory assume about gases?

A
  1. they have a small volume
  2. they dont interact with other gas molecules
  3. move randomly and constantly
  4. engage in elastic collisions
  5. average kinetic energy is equal to absolute temp
39
Q

does one torr equal one mmHg?

A

ya

40
Q

what affects vapor pressure

A

temp, surface area, intermolecular area and solute

41
Q

can gas be soluble in water if the gas is non polar?

A

yea

42
Q

is the pressure of a gas inversely proportional to its temperature in kelvin?

A

no

43
Q

in a spontaneous process, what will always increase?

A

entropy of the universe

44
Q

what doesn’t lead to an increase in entropy?

A

decreasing the volume of a gas

45
Q

the pressure of a gas is inversely proportional to…

A

volume of the gas

46
Q

according to Avogadro’s thing, equal volumes of gas under the same temp and pressure have equal what?

A

number of particles

47
Q

the density of a pure gas at STP depends on its

A

molar mass

48
Q

is the boiling point of pure water always at 100*C?

A

no you stupid bitch

49
Q

what are colligative properties dependent on?

A

relative numbers of solute and solvent particles in a solution

50
Q

what doesn’t cause a system to shift to the right?

A

change in volume (decrease)

51
Q

pure water at any temp has

A

[H3O]=[OH]

52
Q

is HNO3 a strong acid?

A

yes dumbass

53
Q

the degree of ionization of a weak acid

A

varies with concentration and depends on Ka value

54
Q

if K>Q, will the reactants concentration decrease or increase?

A

decrease dumb bitch

55
Q

reduction

A

gains electrons

56
Q

oxidation

A

loses electrons

57
Q

reducing agent

A

species that is oxidized

58
Q

oxidizing agent

A

species that is reduced

59
Q

the more positive E is…

A

the greater the probability that it will be reduced (wants to be reduced)

60
Q

anode

A

electron at which oxidation takes place (-)

61
Q

cathode

A

electron at which reduction takes place (+)

62
Q

what’s on the left of a cell diagram

A

anode

63
Q

whats on the right of a cell diagram

A

cathode

64
Q

driving force behind a spontaneous reaction?

A

motional freedom of particles increasing

65
Q

when in a process always spontaneous?

A

change in H<0 and change in S>0

66
Q

micro states

A

distribution of particles among energy levels

67
Q

enthalpy

A

change in heat (H)

68
Q

entropy

A

how dispersed energy is (S)

69
Q

three types of motion

A

rotational, translational, vibrational

70
Q

integrated rate law

A

change in concentration of a reactant with time

71
Q

units for 0th order

A

M/s

72
Q

units for first order

A

1/s

73
Q

units for 2nd order

A

1/Ms

74
Q

what is energy distribution affected by?

A

molecular motion and volume

75
Q

what remains constant with Gibbs free energy?

A

temp and pressure

76
Q

what does a reaction rate depend on?

A

concentration

77
Q

if something is spontaneous what is the change in G of the system equal to?

A

less than 0

78
Q

equilibrium constant

A

K

79
Q

what does a large K value mean?

A

reaction is product-favored

80
Q

what does chemical equilibrium mean?

A

forward rate=reverse rate

81
Q

what happens when Q>K?

A

reaction occurs in the reverse direction

82
Q

what happens when you change the volume of a gas in a reaction?

A

change the partial pressure

83
Q

what does a decrease in the volume/increase in pressure move the reaction towards?

A

side with the lower number of moles

84
Q

what does an exothermic reaction move the reaction towards?

A

reactants

85
Q

what does an increase in temp do to the direction of a reaction?

A

forwards

86
Q

what are strong acids converted to in water?

A

H3O

87
Q

the more oxygen atoms…

A

the stronger the acid

88
Q

pH buffer

A

weak acid and conjugate base

89
Q

when can the common-ion affect be applied?

A

anytime there’s a buffer

90
Q

equivalence point

A

equal # of moles of acid and base

91
Q

molar solubility symbol

A

S

92
Q

molar solubility units

A

mol/L

93
Q

solubility units

A

g/L or mg/L

94
Q

Q>K

A

precipitate forms

Chem 106 (13 decks)

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